On the solubility of ethyl acetate in water
If you want to study the solubility of ethyl acetate in water, you must understand the properties of the two. Water is a polar solvent, because its molecules have strong polarity, and the electronegativity difference between hydrogen and oxygen is large, so hydrogen bonds are formed, and the attractive force between water-causing molecules is quite strong.

And ethyl acetate is an ester, and its molecular structure contains carbonyl and ethoxy. Carbonyl has a certain polarity, but ethoxy is a non-polar group. On the whole, the polar ethyl acetate is weak.

According to the principle of similar compatibility, those with similar polarity are easily soluble. The strong polarity of water and the weak polarity of ethyl acetate are significantly different, so the solubility of ethyl acetate in water is limited.

Experiments show that under normal temperature, the solubility of ethyl acetate in water is about 8.3g/100mL of water. When the temperature rises, the molecular thermal motion intensifies, the hydrogen bond between water molecules is broken more, and the ethyl acetate molecule is more likely to penetrate into the water molecular gap, and the solubility may increase slightly. However, due to the essential difference in polarity between the two, the increase is not large.

Furthermore, if there are other solutes in the system, it may also affect the solubility of ethyl acetate in water. If salts are added, their solubility can be changed due to the effect of hydrolysis or salinity. If salt ions interact strongly with water molecules, the solubility of water to ethyl acetate is reduced, which is hydrolysis; conversely, if salt ions promote the interaction of ethyl acetate with water, it is salinity.

In summary, the solubility of ethyl acetate in water is subject to various factors such as its polarity with water, temperature, and other solutes in the system. Its solubility in water is limited, but the factors change, and the solubility also changes.